Which of the following compounds is metallic and paramagnetic ?

Options

A. `T_(i)O_(2)`
B. `CrO_(2)`
C. `VO_(2)`
D. `MnO_(2)`

Explanation

To determine which compound is metallic and paramagnetic, we can follow these steps:

### Step 1: Understand the Terms
- **Metallic**: A compound that contains metal elements and exhibits properties typical of metals, such as conductivity and malleability.
- **Paramagnetic**: A substance that has unpaired electrons, which causes it to be attracted to a magnetic field.

### Step 2: Identify the Compounds
Assuming we have a list of compounds (though not provided in the question), we need to analyze each compound to see if it is metallic and if it has unpaired electrons.

### Step 3: Analyze Each Compound
- For each compound, check if it contains metal ions. Common metallic elements include transition metals, alkali metals, and alkaline earth metals.
- Determine the electron configuration of the metal ions in each compound to check for unpaired electrons.

### Step 4: Example Analysis of VO2
- **Compound**: VO2 (Vanadium Dioxide)
- **Metal Ion**: Vanadium (V)
- **Oxidation State**: In VO2, Vanadium is in the +4 oxidation state (V4+).
- **Electron Configuration**: The electron configuration of Vanadium is [Ar] 3d^3 4s^2. In the +4 state, it loses 4 electrons, resulting in [Ar] 3d^1 (one unpaired electron).
- **Conclusion**: Since V4+ has one unpaired electron, VO2 is paramagnetic.

### Step 5: Determine if it is Metallic
- Since VO2 contains Vanadium, a metal, it is classified as a metallic compound.

### Final Answer
The compound that is metallic and paramagnetic is **VO2**.

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